Calculate the total pressure (in atm) exerted by a mixture of 8 g of $O_2$ and 4 g of $H_2$ confined in a 2-litre vessel at $0^0C$. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

In a mixture of three gases with partial pressures of 200 mmHg, 300 mmHg, and 500 mmHg, what is the total pressure of the gas mixture?

10g each of $He$, $Ne$, and $Ar$ are mixed in a container of volume 'V' at 27°C. What is the total pressure exerted by the mixture? (Assume ideal gas behavior. Atomic masses: $He$=4, $Ne$=20, $Ar$=40, R= 0.0821 L atm/mol K)

Choose the correct option for the total pressure (in atm.) in a mixture of 4 g ${O_2}$ and 2 g ${H_2}$ confined in a total volume of one litre at ${0^0}C$ is[Given $R = 0.082{\rm{L}}\,\,{\rm{atm}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}\,{K^{ - 1}},\,T = 273{\rm{K}}$]

Calculate the total pressure in a 10.0 L cylinder which contains 0.4 g helium, 1.6 g oxygen and 1.4 g nitrogen at 27\,^\circ C.

If density of a gas in closed cylinder is $3.5g{L^{ - 1}}$ at 4.1 atm pressure and ${127^0}C$ temperature then molar mass of the gas will be $\left( {R = 0.082\,L\,atm\,{K^{ - 1}}\,mo{l^{ - 1}}} \right)$

A mixture of nitrogen and oxygen gases exerts a total pressure of 1.2 atm. If the partial pressure of nitrogen is 0.8 atm, what is the partial pressure of oxygen according to Dalton's Law?

The density of oxygen gas at ${25^0}C$ is $1.458{\rm{mg}}/{\rm{litre}}$ at one atmosphere. At what pressure will oxygen have the density twice the value?

The pressure and temperature of $4{\rm{d}}{{\rm{m}}^3}$ of carbon dioxide gas are doubled, then the volume of carbon dioxide gas would be

A mixture of 0.5 moles of $O_2$ and 1 mole of $H_2$ is contained in a 1-litre flask at 273 K. Calculate the total pressure (in atm) inside the flask. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

A vessel contains $28$ g of $N_2$ gas and $4$ g of $He$ gas. The total pressure within the vessel is measured to be $30$ bar. What is the partial pressure exerted by the $He$ gas? [Use atomic masses $N = 14, He = 4$]